An Updated Equilibrium MachineEmeric SchultzDescribes a device that can demonstrate equilibrium and the Le Châtelier principle, as well as kinetic and thermodynamic concepts. The device consists of a leaf blower attached to a plastic container divided into two chambers by a barrier of variable size and form. Styrofoam balls can be exchanged across the barrier when various air pressures are applied by the blower.Schultz, Emeric. J. Chem. Educ.2008, 85, 1131.

Equilibrium |

Kinetics |

Thermodynamics

Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) ComplexesRichard S. Herrick, Kenneth V. Mills, and Lisa P. NestorDescribes an experiment that introduces students to integrated rate laws, the search for a mechanism that is consistent with chemical and kinetic data, and the concept of activation barriers and their measurement in a curriculum whose pedagogical philosophy makes the laboratory the center of learning for undergraduates in their first two years of instruction.Herrick, Richard S.; Mills, Kenneth V.; Nestor, Lisa P. J. Chem. Educ.2008, 85, 1120.

Coordination Compounds |

Kinetics |

Mechanisms of Reactions |

Rate Law |

UV-Vis Spectroscopy

Disorder and Chaos: Developing and Teaching an Interdisciplinary Course on Chemical DynamicsSteven G. DesjardinsDescribes an interdisciplinary course for nonscience majors that introduces ideas about mathematical modeling using examples based on pendulums, chemical kinetics, and population dynamics. Students learn about the nature of measurement and prediction through the use of spreadsheet software for the solution of equations and experimental data collection.Desjardins, Steven G. J. Chem. Educ.2008, 85, 1078.

John KrenosMetiu has created a significant set of volumes on undergraduate physical chemistry. The integration of Mathematica and Mathcad workbooks into the four texts provides instructors with an attractive new option in teaching.Krenos, John. J. Chem. Educ.2008, 85, 206.

Quantum Chemistry |

Statistical Mechanics |

Thermodynamics |

Kinetics

Reaction Order Ambiguity in Integrated Rate PlotsJoe LeeThis article provides a theoretical and statistical justification for the necessity of monitoring a reaction to a substantial fraction of completion if integrated rate plots plots are to yield unambiguous orders.Lee, Joe. J. Chem. Educ.2008, 85, 141.

The Chemistry of Paper PreservationHenry A. CarterThis article examines the applications of chemistry to paper preservation. The acid-catalyzed hydrolysis of cellulose accounts for the deterioration of paper in library books and other written records. To combat this threat to our written heritage, new permanent papers have been developed that are relatively chemically stable and undergo a very slow rate of deterioration. Carter, Henry A. J. Chem. Educ.2007, 84, 1937.

Acids / Bases |

Applications of Chemistry |

Aqueous Solution Chemistry |

Free Radicals |

Gas Chromatography |

HPLC |

pH |

Kinetics |

Rate Law

Visualizing the Transition State: A Hands-on Approach to the Arrhenius EquationThomas S. Kuntzleman, Matthew S. Swanson, and Deborah K. SayersPennies and dice are used to simulate the kinetics of two irreversible "reactions" with a hands-on, Monte Carlo approach. Arrhenius plots of the data generated yield activation energies comparable to assigned values and pre-exponential factors close to what would be expected based on the probability of a "reactant" achieving the correct orientation for conversion into "product". A comparison of the values obtained for the pre-exponential factors for the different simulations allows students to semi-quantitatively discuss the orientational requirement that is contained within this factor.Kuntzleman, Thomas S.; Swanson, Matthew S.; Sayers, Deborah K. J. Chem. Educ.2007, 84, 1776.

Kinetics |

Rate Law

A Student Laboratory Experiment Based on the Vitamin C Clock ReactionEd VitzDescribes an adaptation of the vitamin C clock reaction to a student laboratory experiment in which the orders with respect to peroxide and iodide, the rate constant, and the activation energy are determined by the method of initial rates.Vitz, Ed. J. Chem. Educ.2007, 84, 1156.

Consumer Chemistry |

Kinetics |

Mechanisms of Reactions |

Rate Law

Peer-Developed and Peer-Led Labs in General ChemistryLorena Tribe and Kim KostkaDescribes a student-developed and led laboratory curriculum as a model for producing a more student-centered and rich laboratory experience in general chemistry laboratories.Tribe, Lorena; Kostka, Kim. J. Chem. Educ.2007, 84, 1031.

Acids / Bases |

Electrochemistry |

Equilibrium |

Kinetics |

Laboratory Management |

Thermodynamics |

Student-Centered Learning

An Inexpensive Kinetic Study: The Reaction of FD&C Red #3 (Erythrosin B) with HypochloriteMaher M. Henary and Arlene A. RussellStudents use a desktop visible spectrophotometer to quantitatively follow the rate of disappearance of FD&C Red #3 with hypochlorite. The first-order reaction in both dye and bleach yields simple data that students can easily process and graph using spreadsheet software to obtain the rate constant and the rate law.Henary, Maher M.; Russell, Arlene A. J. Chem. Educ.2007, 84, 480.

Dyes / Pigments |

Kinetics |

Rate Law |

UV-Vis Spectroscopy

Applications of Reaction RateKevin CunninghamThis article presents an assignment in which students are to research and report on a chemical reaction whose increased or decreased rate is of practical importance. The assignment is designed to develop and assess a number of valuable skills and understandings, including the ability to write effectively.Cunningham, Kevin. J. Chem. Educ.2007, 84, 430.

Classroom Scale Demonstrations Using Flash Ignition of Carbon NanotubesDean J. Campbell, Kylee E. Korte, Jesse T. McCann, and Younan XiaFlash-initiated combustion of carbon nanotubes can be demonstrated in a large setting using a variety of demonstrations. These demonstrations can also be used to illustrate the importance of surface area in chemical reactions.Campbell, Dean J.; Korte, Kylee E.; McCann, Jesse T.; Xia, Younan. J. Chem. Educ.2006, 83, 1511.

Textbook Deficiencies: Ambiguities in Chemical Kinetics Rates and Rate ConstantsKeith T. Quisenberry and Joel TellinghuisenRecommends that textbook authors make it clear that (i) the reaction rate and rate constant cannot be defined unambiguously without explicitly stating the reaction for which they apply and therefore (ii) the relation between the half-life, which is a physical property of the reaction system, and the rate constant depends upon how the reaction is written.Quisenberry, Keith T.; Tellinghuisen, Joel. J. Chem. Educ.2006, 83, 510.

Steel Wool and Oxygen: How Constant Should a Rate Constant Be?Michiel VogelezangIn the article Steel Wool and Oxygen: A Look at Kinetics, James Gordon and Katherine Chancey describe an experiment about the kinetics between iron and oxygen. Like all good experiments this one is easy to carry out and produces good results. However, the experiment can even have a greater impact with only a small addition.Vogelezang, Michiel. J. Chem. Educ.2006, 83, 214.

Rotational Mobility in a Crystal Studied by Dielectric Relaxation Spectroscopy. An Experiment for the Physical Chemistry LaboratoryMadalena S. C. Dionísio, Hermínio P. Diogo, J. P. S. Farinha, and Joaquim J. Moura-RamosIn this article we present a laboratory experiment for an undergraduate physical chemistry course. The purpose of this experiment is the study of molecular mobility in a crystal using the technique of dielectric relaxation spectroscopy. The experiment illustrates important physical chemistry concepts. The background of the experimental technique deals with the concepts of orientational and induced polarization and frequency-dependent relative permittivity (or dielectric constant). The kinetic concepts of temperature-dependent relaxation time, activation energy, and activation entropy are involved in the concept of molecular mobility. Dionísio, Madalena S. C.; Diogo, Hermínio P.; Farinha, J. P. S.; Moura-Ramos, Joaquim J. J. Chem. Educ.2005, 82, 1355.

Kinetics |

Phases / Phase Transitions / Diagrams |

Solids |

Crystals / Crystallography

Kinetics of Alcohol Dehydrogenase-Catalyzed Oxidation of Ethanol Followed by Visible SpectroscopyKestutis Bendinskas, Christopher DiJiacomo, Allison Krill, and Ed VitzA two-week biochemistry experiment was introduced in the second-semester general chemistry laboratory to study the oxidation of ethanol in vitro in the presence of the enzyme alcohol dehydrogenase (ADH). This reaction should pique student interest because the same reaction also occurs in human bodies when alcoholic drinks are consumed. Procedures were developed to follow the biochemical reaction by visible spectroscopy and to avoid specialized equipment. The effect of substrate concentration on the rate of this enzymatic reaction was investigated during the first week. The effects of temperature, pH, the specificity of the enzyme to several substrates, and the enzyme's inhibition by heavy metals were explored during the second week. Bendinskas, Kestutis; DiJiacomo, Christopher; Krill, Allison; Vitz, Ed. J. Chem. Educ.2005, 82, 1068.

Enzymes |

Kinetics |

Oxidation / Reduction |

Reactions |

UV-Vis Spectroscopy |

Alcohols |

Biophysical Chemistry |

Food Science

Steel Wool and Oxygen: A Look at KineticsJames Gordon and Katherine ChanceyAn experimental method is described to study the kinetics of the reaction of the iron in steel wool with molecular oxygen. A calculator-based data collection system is used with an oxygen gas sensor to determine the order of the reaction with respect to oxygen. Using the graphical method, students determine that the reaction follows first-order kinetics with respect to oxygen. Gordon, James; Chancey, Katherine. J. Chem. Educ.2005, 82, 1065.

Atmospheric Chemistry |

Gases |

Kinetics |

Oxidation / Reduction

A Modified Demonstration of the Catalytic Decomposition of Hydrogen PeroxideCarlos Alexander TrujilloA safer and cheaper version of the popular catalyzed decomposition of hydrogen peroxide demonstration commonly called the Elephants Toothpaste is presented. Hydrogen peroxide is decomposed in the presence of a surfactant by the enzyme catalase producing foam. Catalase has a higher activity compared with the traditional iodide and permits the use of diluted hydrogen peroxide solutions. The demonstration can be made with household products with similar amazing effects. Trujillo, Carlos Alexander. J. Chem. Educ.2005, 82, 855.

Old Nassau Demonstration with Wilkinson ModificationLawrence E. WilkinsonA modification of the Old Nassau Reaction demonstration is presented, wherein a 0.025 M silver nitrate solution is used in place of the mercury(II) chloride solution employed in the original demonstration. Wilkinson, Lawrence E. J. Chem. Educ.2004, 81, 1474.

Aqueous Solution Chemistry |

Kinetics |

Oxidation / Reduction |

Reactions

Using Clinical Cases To Teach General ChemistryBrahmadeo Dewprashad, Charles Kosky, Geraldine S. Vaz, and Charlotte L. MartinThis article describes how a fact-based clinical case was effectively used to motivate and enrich the classroom experience and review many of the concepts covered in general chemistry. The case involves an elderly patient who was brought to the emergency room. The results of his physical examination and laboratory analysis of his blood are presented. The students, in peer-led groups, work through the chemical principles involved in the doctor's diagnosis and treatment options for the patient. The article describes the case study, instructors' observations, and students' perception of the activity. Dewprashad, Brahmadeo; Kosky, Charles; Vaz, Geraldine S.; Martin, Charlotte L. J. Chem. Educ.2004, 81, 1471.

Acids / Bases |

Drugs / Pharmaceuticals |

Equilibrium |

Kinetics |

Medicinal Chemistry

A Simple, Inexpensive Water-Jacketed Cuvette for the Spectronic 20Jonathan E. Thompson and Jason TingA simple, inexpensive, water-jacketed cuvette for the Spectronic 20 is described. The cuvette and associated flow system can easily be constructed from materials commonly found in an undergraduate chemistry laboratory. As a demonstration of the cuvette's utility, we used the cuvette for the determination of the activation energy for the reaction between crystal violet and hydroxide ion. However, the cuvette may prove useful in a variety of applications in which a sample must be thermostated within a spectrophotometer. Thompson, Jonathan E.; Ting, Jason. J. Chem. Educ.2004, 81, 1341.

Kinetics of the Osmotic Hydration of ChickpeasGabriel Pinto and Ali EsinAn experiment examining the swelling of chickpeas as they are soaked in water is presented to introduce students to topics such as osmotic flow, mass transfer, diffusion, kinetics of hydration, modeling, and estimation of activation energy.Pinto, Gabriel; Esin, Ali. J. Chem. Educ.2004, 81, 532.

Kinetics |

Water / Water Chemistry |

Food Science |

Transport Properties

Using a Graphing Calculator To Determine a First-Order Rate Constant: Author ReplyJosé E. Cortés-FigueroaWhen technology is used to help with mathematical calculations, the emphasis must be on the concepts being learned rather than simply the procedures. In our approach we are attempting to help students learn more about the concept and also to attain data analysis skills they will need in the future. Cortés-Figueroa, José E. J. Chem. Educ.2004, 81, 485.

A Modular Laser Apparatus for Polarimetry, Nephelometry, and Fluorimetry in General ChemistryScott A. Darveau, Jessica Mueller, April Vaverka, Cheri Barta, Anthony Fitch, Jessica Jurzenski, and Yvonne GindtWe present an apparatus suitable for multiple uses in the general chemistry laboratory including polarimetry, fluorescence, and nephelometry. The open design of the instrument also decreases the chance that students will contract the "black-box syndrome" that seems to develop when using instruments that only provide the final data in an experiment without showing how the measurements are obtained. Darveau, Scott A.; Mueller, Jessica; Vaverka, April; Barta, Cheri; Fitch, Anthony; Jurzenski, Jessica; Gindt, Yvonne. J. Chem. Educ.2004, 81, 401.

Fluorescence Spectroscopy |

Kinetics |

Laboratory Equipment / Apparatus |

Lasers |

Spectroscopy |

Proteins / Peptides |

Water / Water Chemistry

Why Chemical Reactions Happen (James Keeler and Peter Wothers)John KrenosBy concentrating on a limited number of model reactions, this book presents chemistry as a cohesive whole by tying together the fundamentals of thermodynamics, chemical kinetics, and quantum chemistry, mainly through the use of molecular orbital interpretations. Krenos, John. J. Chem. Educ.2004, 81, 201.

Reactions (→) vs Equations (=)S. R. LoganA recent chemical kinetics text uses an equals sign for an overall reaction, whereas an arrow is used in each of the reaction steps that are proposed to constitute the mechanism, and for any elementary process. Logan, S. R. J. Chem. Educ.2003, 80, 1258.

Factors Affecting Reaction Kinetics of Glucose OxidaseKristin A. JohnsonDemonstration based on a biochemical kinetics experiment in which the rate of reaction varies with the enzyme concentration, substrate concentration, substrate used in the reaction, and temperature. Johnson, Kristin A. J. Chem. Educ.2002, 79, 74.

The State of Division of Solids and Chemical EquilibriaJoão C. M. Paiva and Victor M. S. GilAn experiment and a computer simulation are presented to address a counterintuitive situation often encountered when teaching chemical equilibria. This is prompted by the question "How can the subdivision of a solid reactant affect the reaction rate and not the composition of the equilibrium state?" Paiva, João C. M.; Gil, Victor M. S. J. Chem. Educ.2001, 78, 222.

Equilibrium |

Kinetics |

Laboratory Computing / Interfacing

A Simple Method for Demonstrating Enzyme Kinetics Using Catalase from Beef Liver ExtractKristin A. JohnsonA simple visual method of demonstrating enzyme kinetics using beef liver catalase. Filter paper is saturated with beef liver extract and placed into a solution of hydrogen peroxide. The catalase in the extract decomposes the hydrogen peroxide to water and oxygen. Oxygen forms on the filter paper, and the filter paper rises to the top of the beaker. Catalase activity is measured by timing the rise of the enzyme-soaked filter paper to the top of beakers containing different concentrations of hydrogen peroxide. Johnson, A. Kristin. J. Chem. Educ.2000, 77, 1451.

Enzymes |

Kinetics |

Proteins / Peptides |

Reactions

Epoxy PolymerizationFred Schubert and Tom LoBuglioIdentifying the gel point of a polymer using a multimeter.Schubert, Fred; LoBuglio, Tom. J. Chem. Educ.2000, 77, 1409.

Comparisons and Demonstrations of Scientific CalculatorsMyung-Hoon Kim, Suw-Young Ly, and Tae-Kee HongScientific calculators are compared in terms of their capacities, featuring many advantages of the graphic calculator over simple nongraphic calculators. Applications in this paper include a simulation of acid-base titration curves, and graphic display of a time course of concentrations of reactants and products for a chemical reaction with first-order kinetics.Kim, Myung-Hoon; Ly, Suw-Young; Hong, Tae-Kee. J. Chem. Educ.2000, 77, 1367.

Every Year Begins a MillenniumJerry A. BellThis article outlines a series of demonstrations and their contexts, leading to recommendations about what we teach and how we teach.Bell, Jerry A. J. Chem. Educ.2000, 77, 1098.

Acids / Bases |

Aqueous Solution Chemistry |

Equilibrium |

Kinetics |

Learning Theories

Paradoxes, Puzzles, and Pitfalls of Incomplete Combustion DemonstrationsEd VitzPaper is burned in a closed container containing sufficient oxygen to consume all the paper. Paradoxically, the flame expires while half of the paper remains. This demonstrates that thermodynamics or stoichiometry is insufficient to explain everyday chemical processes, and that kinetics is often necessary. The gases in the container are analyzed by GC before and after combustion, and the results are examined in detail. Vitz, Ed. J. Chem. Educ.2000, 77, 1011.

Gases |

Kinetics |

Stoichiometry

Modeling Chemical Processes in Seawater Aquaria to Illustrate Concepts in Undergraduate ChemistryGordan GrguricThis paper describes three exercises which can be used in a variety of undergraduate chemistry curricula: (i) determining the salts and their amounts needed to prepare a given volume of artificial seawater, (ii) modeling aqueous carbonate equilibria, to calculate pH and alkalinity shifts through additions of chemicals, and (iii) modeling chemical kinetics involved in aqueous ozone-bromine reactions, to predict the type and extent of disinfection by-products. Grguric, Gordan. J. Chem. Educ.2000, 77, 495.

Aqueous Solution Chemistry |

Equilibrium |

Kinetics |

Applications of Chemistry

Experiments with AspirinLonda L. Borer and Edward BarryExperiments include (i) synthesis, purification, and characterization of aspirin by mp and TLC, (ii) percentage composition of a commercial aspirin tablet by titration, (iii) kinetics of the hydrolysis of aspirin to salicylic acid under various conditions, (iv) synthesis and characterization of copper(II) aspirinate and copper(II) salicylate, and (v) reaction of copper(II) aspirinate in aqueous solution. Borer, Londa L.; Barry, Edward. J. Chem. Educ.2000, 77, 354.

Synthesis |

Kinetics |

Drugs / Pharmaceuticals |

Medicinal Chemistry |

Aromatic Compounds

The Blue Bottle Reaction as a General Chemistry Experiment on Reaction MechanismsSteven C. Engerer and A. Gilbert CookUsing the scientific method (observe, question, hypothesize, experiment, repeat) students propose and test possible reaction mechanisms for the methylene blue-catalyzed oxidation of dextrose with its dramatic color change. Students are led to discover the three-step mechanism through a series of questions.Engerer, Steven C.; Cook, A. Gilbert. J. Chem. Educ.1999, 76, 1519.

Old Rule of Thumb and the Arrhenius EquationI. A. LeensonThe empirical rule (doubling of the reaction rate upon every 10 increase in temperature) is discussed on the basis of the Arrhenius equation and experimental data. A graph is plotted that shows the applicability limits of the empirical rule in terms of activation energies and temperatures. Leenson, Ilya A. J. Chem. Educ.1999, 76, 1459.

Using CBL Technology and a Graphing Calculator To Teach the Kinetics of Consecutive First-Order ReactionsJosé E. Cortés-Figueroa and Deborah A. MooreThis work proposes a demonstration to introduce first-order reactions using the CBL system. It then presents the analysis of two consecutive first-order reactions. The values of the rate constants that govern each reaction's rate are determined using the graphing and statistical capabilities of a TI-83 calculator. Cortés-Figueroa, José E.; Moore, Deborah A. J. Chem. Educ.1999, 76, 635.

Kinetics |

Laboratory Computing / Interfacing |

Rate Law

A New Twist on the Iodine Clock Reaction: Determining the Order of a ReactionXavier Creary and Karen M. MorrisThe iodine clock reaction can be used to illustrate the kinetic order of a reaction, and an overhead projector demonstration was developed three years ago for general chemistry classes at the University of Notre Dame showing this concept. Creary, Xavier; Morris, Karen M. J. Chem. Educ.1999, 76, 530.

Aqueous Solution Chemistry |

Kinetics

Equilibrium Principles: A Game for StudentsLionel J. Edmonson Jr. and Don L. LewisThe laboratory exercise is a game using marked sugar cubes as dice. The game emphasizes the dynamic character of equilibrium. Forward and reverse rate-constant values are used to calculate an equilibrium constant and to predict equilibrium populations. Predicted equilibrium populations are compared with experimental results.Edmonson, Lionel J., Jr.; Lewis, Don L. J. Chem. Educ.1999, 76, 502.

The Fizz Keeper, a Case Study in Chemical Education, Equilibrium, and KineticsReed HowaldThe chemistry of the loss of carbonation from carbonated beverages on storage is considered. Increasing the pressure of CO2(g) will restore carbonation, but an increase in pressure adding air should not affect the equilibria. It can and does, however, affect the kinetics-the rate at which a new equilibrium is established. Thus the Fizz Keeper is effective for storage of resealed pop containers for hours, but not for periods of weeks or months. Howald, Reed. J. Chem. Educ.1999, 76, 208.

A Simple Method To Demonstrate the Enzymatic Production of Hydrogen from SugarNatalie Hershlag, Ian Hurley, and Jonathan WoodwardIn the experimental protocol described here, it has been demonstrated that the common sugar glucose can be used to produce hydrogen using two enzymes, glucose dehydrogenase and hydrogenase. No sophisticated or expensive hydrogen detection equipment is required-only a redox dye, benzyl viologen, which turns purple when it is reduced. The color can be detected by a simple colorimeter. Hershlag, Natalie; Hurley, Ian; Woodward, Jonathan. J. Chem. Educ.1998, 75, 1270.

Enzymes |

Kinetics |

UV-Vis Spectroscopy |

Carbohydrates |

Applications of Chemistry

Why the Arrhenius Equation Is Always in the "Exponentially Increasing" Region in Chemical Kinetic StudiesHarvey F. CarrollThe Arrhenius equation in chemical kinetics, k = Ae-Ea/RT, has, as T gets larger, an inflection point where it changes from an "exponentially increasing" curve to one approaching an asymptote of A. The inflection point occurs at T = Ea/2R. For any activation energy, the inflection point occurs at such a high temperature that chemical kinetic studies would not be possible. Thus, the Arrhenius equation always appears to be exponentially increasing in any chemical kinetic studies of interest. Carroll, Harvey F. J. Chem. Educ.1998, 75, 1186.

Kinetics

The Reaction of a Food Colorant with Sodium Hypochlorite: A Student-Designed Kinetics ExperimentJosefina Arce, Rosa Betancourt, Yamil Rivera, and Joan PijemThe kinetics of the reaction of the food colorant FD&C Blue #1 with sodium hypochlorite (Clorox) is described in a student-designed experimental format. In this format, students are guided- by means of questions- to make decisions regarding concentration of reagents, choice of equipment, and actual laboratory procedures to be followed. Arce, Josefina; Betancourt-Perez, Rosa; Rivera, Yamil; Pijem, Joan. J. Chem. Educ.1998, 75, 1142.

Kinetics |

UV-Vis Spectroscopy |

Dyes / Pigments

Chemistry Time: Factors Affecting the Rate of a Chemical ReactionThis activity can be used to introduce a unit on chemical kinetics, but it is simple enough to be used in a discussion of chemical reactions or experimental methods/procedures during the first weeks of the semester. The activity involves reacting bicarbonate with acid, a reaction with practical applications in everyday life.J. Chem. Educ.1998, 75, 1120A.

Kinetics |

Rate Law

Limiting Reagent and Kinetics: Social Implications and Malthus' PredictionL. H. Holmes Jr.Robert Malthus predicted in the early 1800s that man would outstrip his food supply. The amount of carbon on earth is the ultimate limiting reagent for the number of people the earth can have and in the sense that carbon is our "food", Malthus was right. However, the land area of the earth is a "limiting reagent" that will limit our population before carbon does. These concepts are discussed in the context of limiting reagents and chemical kinetics to show that if the rate of increase of population remains at what it is now, we have less than a thousand years to "solve" the problem. Holmes, L. H., Jr. J. Chem. Educ.1998, 75, 1004.

Kinetics

Ernest Rutherford, Avogadro's Number, and Chemical KineticsI. A. LeensonThe paper presents a way for students to use data from Rutherford's works (1908 - 1911) in order to determine one of the most precise values of Avogadro Constant available at the beginning of the century. Leenson, I. A. J. Chem. Educ.1998, 75, 998.

Learning Theories |

Nuclear / Radiochemistry |

Kinetics

Audience-Appropriate Analogies: Collision TheoryKent W. PiepgrassThis article presents two new analogies for collision theory based on arcade games and on the interactions between salesclerks and customers in a store. The uses, limitations, and possible extensions of the analogies are discussed. Piepgrass, Kent W. J. Chem. Educ.1998, 75, 724.

Learning Theories |

Mechanisms of Reactions |

Kinetics

An Analogy to Help Students Understand Reaction OrdersCharles J. MarzzaccoThis article describes a simple analogy to help students understand the concept of the rate law for a chemical reaction. The analogy involves the mathematical relationships between various characteristics of a cube and the length of its edge. Charles J. Marzzacco. J. Chem. Educ.1998, 75, 482.

Dice Shaking as an Analogy for Radioactive Decay and First Order KineticsEmeric SchultzAn experiment involving the shaking of sets of different sided dice is described. Dice of 4, 6, 8, 10, 12 and 20 sides are readily available. This experiment serves as an easily understood analogy for radioactive decay and for the more general case of first order kinetics. Schultz, Emeric. J. Chem. Educ.1997, 74, 505.

SIRS: Simulations and Interactive Resources, IIIMartin, John S.Simulations and Interactive Resources (SIRs) are designed to support interactive lectures in introductory chemistry. This third issue of SIRs includes five new SIRs as well as updated and final versions of all previously published SIRs.Martin, John S. J. Chem. Educ.1996, 73, 722.

Periodicity / Periodic Table |

Equilibrium |

Gases |

Thermodynamics |

Reactions |

Electrochemistry |

Kinetics

Reduction of Viologen Bisphosphonate Dihalide with Aluminum FoilPeter Abeta IyereAn elegant undergraduate experiment similar to the popular "Iodine Clock Reaction" employs the reduction of methyl viologen by hydroxide ion. This demonstration can be used as prelaboratory discussion for an undergraduate kinetic experiment based on the same phenomenon.Iyere, Peter Abeta. J. Chem. Educ.1996, 73, 455.

Kinetics |

Equilibrium

Lightstick Magic: Determination of the Activation Energy with PSLThomas H. BindelThe energy of activation of the light-producing reaction in a lightstick is determined in two different ways. Each depends upon a computer-assisted collection of data from both a light probe and temperature probe. One of them is novel in that data is collected under nonisothermal conditions. Bindel, Thomas H. J. Chem. Educ.1996, 73, 356.

Curve Fitting: An Alternative Approach to Analyzing Kinetic Data in Introductory ChemistryColeman, William F.183. The availability of high quality software for performing nonlinear curve fitting on microcomputers allows students to take an alternative approach to data analysis, one that concentrates on functional forms that may be more natural than some of the algebraic machinations necessary to render relationships into linear forms. An example of the application of such an approach to the analysis of kinetic data is presented in this paper.Coleman, William F. J. Chem. Educ.1996, 73, 243.

Simple and inexpensive kinetics: A student laboratory experiment and demonstration Erwin, David K.Laboratory experimentation, as well as in-class demonstration, involving the study of chemical kinetics can be performed using this safe, simple, and inexpensive apparatus. This apparatus requires only that systems to be studied must produce a gaseous product that can displace water.Erwin, David K. J. Chem. Educ.1992, 69, 926.

A simple second-order kinetics experimentWeiss, Hilton M.; Touchette, KimThe reaction studied in this experiment is the (reversible) dimerization of 2,5-dimethyl-3,4-diphenylcyclopentadienone; the monomer is colored while the dimer is not, so monitoring the reaction with a simple spectrophotometer provides the concentration of the monomer and therefore the rate of its disappearance.Weiss, Hilton M.; Touchette, Kim J. Chem. Educ.1990, 67, 707.

Reduction of permanganate: A kinetics demonstration for general chemistrySteffel, Margaret J.Using the reduction of MnO4- to Mn2+ in aqueous solution to demonstrate the four factors that control reaction rates in solution: the natures of the reactants, concentrations of the reactants, temperature, and the presence of a catalyst.Steffel, Margaret J. J. Chem. Educ.1990, 67, 598.

Kinetics |

Rate Law |

Catalysis |

Oxidation / Reduction

Wet labs, computers, and spreadsheetsDurham, BillThe following is a description of some commonly encountered experiments that have been modified for computerized data acquisition.Durham, Bill J. Chem. Educ.1990, 67, 416.

Laboratory Computing / Interfacing |

Nuclear / Radiochemistry |

Titration / Volumetric Analysis |

Calorimetry / Thermochemistry |

Kinetics |

Electrochemistry

An effective approach to teaching electrochemistryBirss, Viola I.; Truax, D. RodneyBy interweaving concepts from thermodynamics and chemical kinetics with those of electrochemical measurement, the authors provide students with an enriched appreciation of the utility of ideas from kinetics and thermodynamics.Birss, Viola I.; Truax, D. Rodney J. Chem. Educ.1990, 67, 403.

Electrochemistry |

Kinetics |

Thermodynamics

Polarized light and rates of chemical reactionsWeir, John J.This experiment provides the opportunity to introduce the principles of reaction kinetics, polarized light, and the chemistry of optically active compounds; the rate of the acid-catalyzed hydrolysis of sucrose to glucose and fructose is determined.Weir, John J. J. Chem. Educ.1989, 66, 1035.

Rate Law |

Kinetics |

Chirality / Optical Activity |

Carboxylic Acids

Computer simulation of chemical equilibriumCullen, John F., Jr.108. The "Great Chemical Bead Game" requires no instruments and presents the concepts of equilibrium and kinetics more clearly than an experiment. [October and November Computer Series both inadvertently called number 107. Numbering restored by skipping 109 and calling January 1990 number 110.]Cullen, John F., Jr. J. Chem. Educ.1989, 66, 1023.

Analysis of kinetic data with a spreadsheet programHenderson, JohnAn article about spreadsheet templates that accept concentration versus time data for several runs of an experiment, determination of least-squares lines through data points for each run, and will allow the user to exclude points from the least-squares calculation.Henderson, John J. Chem. Educ.1988, 65, A150.

Some analogies for teaching rates/equilibrium Olney, David J.This article presents several analogies for teaching rates and equilibrium developed by the author over his many years in the chemistry classroom that seem to be effective.Olney, David J. J. Chem. Educ.1988, 65, 696.

Kinetics |

Equilibrium

A "stationery" kinetics experiment Hall, L.; Goherdhansingh, A.The simple redox reaction that occurs between potassium permanganate and oxalic acid can be used to prepare an interesting disappearing ink that is the basis for a kinetics experiment for an introductory chemistry class.Hall, L.; Goherdhansingh, A. J. Chem. Educ.1988, 65, 142.

Enthalpy and Hot Wheels: An analogyBonneau, Marcia C.Demonstrating the relationship between activation energy and the heat of a reaction using a "Hot Wheels" track and car to simulate a potential energy diagram.Bonneau, Marcia C. J. Chem. Educ.1987, 64, 486.

Kinetics |

Calorimetry / Thermochemistry |

Thermodynamics

The cola clock: A new flavor to an old classicRussell, Richard A.; Switzer, Robert W.The classic iodine clock reaction with Vitex replacing starch as the indicator.Russell, Richard A.; Switzer, Robert W. J. Chem. Educ.1987, 64, 445.

Change in concentration with timeUmland, Jean B.Shows how the rate of a reaction is fast at first and then gradually decreases to zero when one reactant has been used up.Umland, Jean B. J. Chem. Educ.1985, 62, 153.

Thermodynamic changes, kinetics, equilibrium, and LeChatelier's principleHansen, Robert C.A series of demonstrations in which water in beakers and the flow of water between beakers is used to represent the components of an exothermic chemical reaction and the flow and quantity of thermal energy involved in chemical changes.Hansen, Robert C. J. Chem. Educ.1984, 61, 804.

Cooking with chemistryGrosser, Arthur E.Two demonstrations involving cooking eggs and suggestions for many more examples of cooking that illustrate important principles of chemistry. From the "State-of-the-Art Symposium for Chemical Educators: Chemistry of the Food Cycle".Grosser, Arthur E. J. Chem. Educ.1984, 61, 362.

Computer simulation of elementary chemical kinetics Nase, Martha L.; Seidman, Kurt44. Bits and pieces, 16. The authors have developed several computer programs that simulate chemical kinetics for elementary first and second order processes. These programs can be used to generate kinetic data that can then be analyzed by the student in a variety of ways.Nase, Martha L.; Seidman, Kurt J. Chem. Educ.1983, 60, 734.

Getting a "bang" out of chemical kineticsHague, George R., Jr.The kinetics demonstration described in this note has attracted as many as 15,000people to come and watch.Hague, George R., Jr. J. Chem. Educ.1983, 60, 355.

What is the rate-limiting step of a multistep reaction?Murdoch, Joseph R.The purpose of this paper is to point out the circumstances where analogies can be used successfully and to develop a generalization which can be used for all reactions, including those with polymolecular steps.Murdoch, Joseph R. J. Chem. Educ.1981, 58, 32.

The kinetics of runningLarsen, Russell D.The consideration of running as a rate process has several advantages for a student studying chemical kinetics for the first time.Larsen, Russell D. J. Chem. Educ.1979, 56, 651.

Kinetics |

Rate Law

The temperature dependence of the equilibrium constantBurness, James H.This exam question tests a student's ability to derive the temperature dependence of an equilibrium constant not by qualitatively applying Le Chatelier's principle, but by understanding the relationship between the kinetics of the equation and the value of Keq.Burness, James H. J. Chem. Educ.1979, 56, 395.

Reaction rates for a homogeneously catalyzed reactionNechamkin, Howard; Keller, Elhannan; Goodkin, JeromeThe reaction of KMnO4 with hydrogen in an acidic medium is an example of a homogeneously catalyzed reaction that can be performed by college freshmen.Nechamkin, Howard; Keller, Elhannan; Goodkin, Jerome J. Chem. Educ.1977, 54, 775.

Rate Law |

Kinetics |

Catalysis

Water dipping kinetics. A physical analog for chemical kineticsBirk, James P.; Gunter, S. KayPhysical analogs of zero-, first, and second-order kinetics using the volume of water transferred by a dipper oriented in different directions with respect to a basin of water.Birk, James P.; Gunter, S. Kay J. Chem. Educ.1977, 54, 557.

Pseudo first-order kineticsCorbett, John F.A kinetic study of second-order reactions under first-order conditions can yield accurate second-order rate constants provided an empirical allowance is made for the depletion of the reactant in excess.Corbett, John F. J. Chem. Educ.1972, 49, 663.

A study of the physical and chemical rates of CaCO3 dissolution in HClBassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, BenThe authors describe the experimental procedure and a discussion of results for a study of the physical and chemical rates of CaCO3 dissolution in HCl.Bassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, Ben J. Chem. Educ.1971, 48, 327.

Acids / Bases |

Kinetics |

Reactions |

Rate Law

MiscellaneousAlyea, Hubert N.These twelve overhead projection demonstrations include rates of reactions, clock reactions, the effect of temperature and the presence of a catalyst on the decomposition of hydrogen peroxide, the relationship between viscosity and temperature, equilibria, solubility product, and the common ion effect.Alyea, Hubert N. J. Chem. Educ.1970, 47, A437.

Hydrolysis of benzenediazonium ionSheats, John E.; Harbison, Kenneth G.Presents a more convenient approach to studying the kinetics of the hydrolysis of benzenediazonium ion.Sheats, John E.; Harbison, Kenneth G. J. Chem. Educ.1970, 47, 779.

Aromatic Compounds |

Nucleophilic Substitution |

Kinetics

Prolonging death (in apples)Plumb, Robert C.Using controlled atmosphere storage to prolong the freshness of vegetables and fruits after they have been harvested.Plumb, Robert C. J. Chem. Educ.1970, 47, 518.

Equilibrium |

Kinetics |

Agricultural Chemistry |

Applications of Chemistry |

Gases

The Methanol LighterBailar, John C., Jr.The methanol lighter illustrates the roles that thermodynamics, kinetics, and catalysis play in determining if a reaction will take place.Bailar, John C., Jr. J. Chem. Educ.1970, 47, 272.

The law of mass actionBerline, Steven; Bricker, ClarkIt is the purpose of this paper to present a derivation of the Law of Mass Action that should have meaning and could be used at an elementary level.Berline, Steven; Bricker, Clark J. Chem. Educ.1969, 46, 499.

Probabilistic derivation of the kinetic rate equationsLee, Tieh-Sheng; Kuffner, Roy J.The use of the probabilistic approach is readily applicable to reaction kinetics if one considers the probability of the survival of the reactant molecule instead of the survival of a radioactive nucleus.Lee, Tieh-Sheng; Kuffner, Roy J. J. Chem. Educ.1968, 45, 430.

Kinetics

Bimolecular nucleophilic displacement reactionsEdwards, John O.The bimolecular nucleophilic displacement reaction is important and should be included in any detailed discussion of kinetics and mechanism at an early undergraduate level.Edwards, John O. J. Chem. Educ.1968, 45, 386.

Reactions |

Nucleophilic Substitution |

Kinetics |

Mechanisms of Reactions

From stoichiometry and rate law to mechanismEdwards, John O.; Greene, Edward F.; Ross, JohnExamines the rules used by chemists as guidelines in developing mechanisms from stoichiometric and rate law observations. Edwards, John O.; Greene, Edward F.; Ross, John J. Chem. Educ.1968, 45, 381.

Stoichiometry |

Rate Law |

Kinetics |

Mechanisms of Reactions |

Equilibrium |

Reactive Intermediates

The revolution in elementary kinetics and freshman chemistryWolfgang, RichardNew developments in kinetics so fundamentally affect our most elementary conception of chemical change that they must inevitably be reflected in beginning courses in chemistry; includes an outline for freshmen on elementary chemical dynamics.Wolfgang, Richard J. Chem. Educ.1968, 45, 359.

Alcohols to alkyl halides: A kinetics experiment for elementary chemistry coursesCooley, J. H.; McCown, J. D.; Shill, R. M.The rate measurement in this procedure is accomplished by direct observation of the change in length or volume of the insoluble layer of an alkyl bromide that is formed from a mixture of alcohol, hydrobromic acid, and sulfuric acid.Cooley, J. H.; McCown, J. D.; Shill, R. M. J. Chem. Educ.1967, 44, 280.

Alcohols |

Synthesis |

Kinetics |

Rate Law

The dissolution of tin in solutions of iodineDavies, J. F.; Trotman-Dickenson, A. F.The progress of this reaction can be followed by the loss of weight of a tin disc.Davies, J. F.; Trotman-Dickenson, A. F. J. Chem. Educ.1966, 43, 483.

A kinetics experiment for first year chemistryShaefer, William P.The exchange of iodine atoms between organic and inorganic iodides serves as a kinetics experiment for first year chemistry.Shaefer, William P. J. Chem. Educ.1964, 41, 558.

Kinetics |

Isotopes |

Rate Law

The oxidation of iodide ion by persulfate ionMoews, P. C., Jr.; Petrucci, R. H.Presents the oxidation of iodide ion by persulfate ion as an ideal reaction to study as part of an experiment on kinetics.Moews, P. C., Jr.; Petrucci, R. H. J. Chem. Educ.1964, 41, 549.

Principles of chemical reactionSanderson, R. T.The purpose of this paper is to examine the nature of chemical change in the hope of recognizing and setting forth the basic principles that help us to understand why they occur.Sanderson, R. T. J. Chem. Educ.1964, 41, 13.

A kinetic analogyLemlich, RobertThis analogy, which clearly demonstrates the principles involved in a first-order reaction, is based on Poiseuille's law for the viscous flow of fluids.Lemlich, Robert J. Chem. Educ.1954, 31, 431.